Boyle's Law describes the relationship between pressure and volume of gas when:

Boyle's Law states that the pressure of a gas is inversely proportional to its volume when the temperature remains constant. This means that if you decrease the volume of a gas, the pressure will increase, provided that the temperature does not change. This principle is essential in various scientific and practical applications, such as understanding how pistons work in engines or the behavior of gases in different environmental conditions.

When temperature is constant, any changes in volume will directly affect the pressure, which is the core concept of Boyle's Law. For example, if air is compressed into a smaller space, the molecules have less room to move, resulting in an increased number of collisions with the walls of the container, thereby raising the pressure.

Knowing this relationship is critical for safe and effective applications in fields like diving, where gas laws govern how divers must manage gas supplies and pressures to avoid problems like decompression sickness.